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Chemistry 121 > notes 23-34 > Flashcards

notes 23-34 Flashcards

1
Q

Aufbau Principle

A

as protons are added on by one to the nucleus to build up the elements, electrons are similarly added to these hydrogen-like orbitals

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2
Q

Hund’s Rule

A

the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons (upe) allowed by the Pauli principle in a particular set of degenerate orbitals; generally shown as spin up

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3
Q

Pauli Exclusion Principle

A

no two electrons in an atom can have the same four numbers; electrons in the same orbital must have opposite spins

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4
Q

valence electrons (ve)

A

the electrons in the outermost principal quantum level of an atom

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5
Q

core electrons

A

inner electrons

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6
Q

Elements that have the same number of valence electrons…

A

…are in the same group which is why they have similar chemical reactivity.

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7
Q

Atomic Radius trend

A

atomic radii increases down a group and decreases across a period

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8
Q

Ionization Energy (IE)

A

the energy required to completely remove an electron from a gaseous atom or ion

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9
Q

Ionization Energy trend

A

IE decreases down a group and increases across a period (larger n → larger size → smaller IE)

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10
Q

Electron Affinity

A

the energy change associated with the addition of an electron to a gaseous atom

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11
Q

The greater the electron affinity…

A

…the greater the energy released when the electron is “captured” by the atom.

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12
Q

Electron Affinity trend

A

the electron affinity decreases (less negative) down a group and increases (more negative) across a period

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13
Q

Electron Affinity trend exceptions

A

He, Be, N, Ne, Mg, Ar

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14
Q

Size of Ions trend

A
  1. cations are smaller than the parent ion (removing electrons)
  2. anions are larger than the parent ion (adding electrons)
  3. ion size increases down a group
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15
Q

Isoelectronic Ions

A

ions containing the same number of electrons

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16
Q

Isoelectronic Ions trend

A

as atomic number increases the ionic radii decreases for an isoelectronic series

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17
Q

Paramagnetism

A

causes the substance to be attracted into an induced magnetic field; unpaired electrons

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18
Q

Diamagnetism

A

causes the substance to be repelled from an induced magnetic field; paired electrons

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19
Q

Metallic Character

A

metallic character increases down a group and decreases across a period

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20
Q

Bond Energy

A

the energy required to break a bond

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21
Q

ionic bonding

A

an atom loses electrons relatively easily and reacts with an atom that has a high affinity for that electron

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22
Q

covalent bonding

A

electrons are shared by two nuclei

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23
Q

polar covalent bonding

A

unequal sharing of electrons between two atoms

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24
Q

Electronegativity

A

the ability of an atom in a molecule to attract shared electrons to itself

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25
Electronegativity trend
electronegativity decreases down a group and increases across a period; F has the highest electronegativity
26
dipole moment
a measure of the separation of positive and negative charge in a molecule
27
lattice energy
the change in energy that takes place when separated gaseous ions are packed together to form an ionic solid
28
single bond
a shared electron pair (sigma)
29
double bond
two shared electron pairs (sigma + pi)
30
triple bond
three shared electron pairs (sigma + 2pi)
31
C-C bond length
154pm
32
C=C bond length
134pm
33
C≡C bond length
120pm
34
enthalpy equation
ΔH = (sum of bonds broken) - (sum of bonds formed)
35
localized electron (LE) bonding model
a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
36
lone pairs
pairs of electrons localized on an atom
37
bonding pairs
pairs of electrons found between atoms
38
Lewis structure
the arrangement of only the valence electrons in a molecule
39
duet rule
H forms stable molecules where it shares 2ve
40
He doesn't form bonds since...
...it already has 2ve (1s2)
41
octet rule
the 2nd period forms bonds to fill all of its valence orbitals, tend to seek 8ve
42
octet rule deficient
B, Be, Li
43
elements that HAVE to follow the octet rule
C, N, O, F
44
exceeds octet rule
elements in the 3rd period and larger
45
resonance structures
multiple valid Lewis structures for a molecule; the average/combination of all of them is the correct structure
46
formal charge
the difference between the # of valence electrons on the free atom and the # of ve assigned to the atom in the molecule
47
molecular structure
the 3D arrangement of the atoms in a molecule
48
sp hyrbidized
two effective pairs around an atom (one s and one p orbital)
49
dsp3 hybridization
only happens when the octet is violated for the central atom (one d, one s, and three p orbitals)
50
d2sp3 hybridization
six effective pairs around an atom; always arranged octahedrally
51
weaknesses in the LE model
difficulty with uneven number of electrons, representing delocalized electrons, bond energy
52
molecular orbital theory
an advanced model of chemical bonding in which electrons reside in molecular orbitals delocalized over the entire molecule. In the simplest version, the molecular orbitals are simply linear combinations of atomic orbitals
53
MO1 is... MO2 is...
...the sigma bond (bonding orbital) ...the sigma* bond (antibonding orbital)
54
in the molecule the atomic orbitals no longer exist...
...only the MOs exist (new molecule → new orbitals)
55
(bonding) MO1 is... (antibonding) MO2 is...
... lower in energy than either of the two H 1s atomic orbitals ... higher in energy than either of the two H 1s atomic orbitals
56
the MO labels show...
...shape, parent atomic orbitals, and bonding or antibonding
57
bond order (BO)
the difference between the number of bonding electrons and the number of antibonding electrons divided by 2
58
intramolecular forces
forces that bond atoms together to make molecules
59
condensed states of matter
solids and liquids
60
intermolecular forces
forces that hold the molecules together as aggregates
61
gas
low density, indefinite shape, indefinite volume, weak IMF
62
liquid
high density, indefinite shape, definite volume, moderate IMF
63
solid
high density, definite shape, definite volume, strong IMF
64
London Dispersion Forces (LDF)
the forces that exist between nonpolar molecules and atoms
65
polarizability
a measure of how easily the electron cloud of an element can be distorted to give a dipolar charge distribution
66
dipole-dipole attraction
molecules with dipole moments can line up +-+- to attract one another electrostatically
67
hydrogen bonding
occurs in molecules that have hydrogen covalently bonded to highly electronegative atoms (H bonded to F, O, or N)
68
ion-dipole forces
occur when ionic compounds are dissolved in polar substances
69
surface tension
the resistance of a liquid to an increase in its surface area
70
viscosity
a measure of a liquid's resistance to flow
71
capillary action
the spontaneous rising of a liquid in a narrow tube (cohesive + adhesive forces)
72
cohesive forces
a result of the IMF among the molecules of the liquid
73
adhesive forces
the forces between the liquid molecules and the container walls
74
vaporization (evaporation)
when molecules or atoms of a liquid escape the liquid's surface and form a gas
75
enthalpy/heat of vaporization
the energy required to vaporize 1mol of a liquid at 1atm
76
condensation
the process by which vapors reform a liquid
77
vapor pressure
the pressure above the liquid in this closed system at this dynamic equilibrium
78
volatile (VOC's)
liquids with high vapor pressures
79
non-volatile
liquids with low vapor pressures
80
normal boiling point
the temperature at which the vapor pressure of the liquid is exactly 1atm
81
boiling point
the temperature at which the vapor pressure of the liquid is equal to atmospheric pressure (changes with external pressure)
82
Clausius-Clapeyron equation
y=mx+b
83
sublimation
when a solid goes directly to the gaseous state without passing through the liquid state
84
deposition (desublimation)
when a gas goes directly to the solid state without passing through the liquid state
85
heating curve
a plot of temperature vs time for a process where energy is added as a constant rate
86
enthalpy/heat of fusion
the enthalpy change that occurs at the melting point when a solid melts
87
normal melting point
the temperature at which the solid and liquid states have the same vapor pressure under conditions where the total pressure is 1atm
88
superheating
when a liquid is raised to a temperature above its boiling point without boiling
89
sites of nucleation
molecular imperfection where molecules to accumulate
90
bumping
once a bubble forms
91
supercooling
cooled below its freezing point and remain a liquid
92
cooling curve
a plot of temperature vs time for a process where energy is removed as a constant rate
93
phase diagram
a convenient way of representing the phases of substance as a function of temperature and pressure
94
critical temperature
the temperature above which the vapor cannot be liquefied no matter what pressure is applied (376ºC for water)
95
critical pressure
the pressure required to produce liquefaction at the critical temperature (218atm for water)
96
phase diagrams
a convenient way of representing the phases of a substance as a function of temperature and pressure

Chemistry 121 (6 decks)

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